1. Chemistry 19.3

2. Strengths of Acids and Bases
19.3
Lemons and grapefruits have a sour taste because they contain citric acid. Sulfuric acid is a widely used industrial chemical that can quickly cause severe burns if it comes into contact with skin. You will learn why some acids are weak and some acids are strong.

3. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases
Strong and Weak Acids and Bases
How does the value of an acid dissociation constant relate to the strength of an acid?

4. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases
An acid dissociation constant (Ka) is the ratio of the concentration of the dissociated (or ionized) form of an acid to the concentration of the undissociated (nonionized) form.

5. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases
Weak acids have small Ka values. The stronger an acid is, the larger is its Ka value.

6. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases
Strong acids are completely ionized in aqueous solution.
Weak acids ionize only slightly in aqueous solution.

7. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases
In general, the base dissociation constant (Kb) is the ratio of the concentration of the conjugate acid times the concentration of the hydroxide ion to the concentration of the base.

8. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases
Strong bases dissociate completely into metal ions and hydroxide ions in aqueous solution.
Weak bases react with water to form the hydroxide ion and the conjugate acid of the base.

9. Strong and Weak Acids and Bases
19.3
Strong and Weak Acids and Bases

10. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants
Calculating Dissociation Constants
How can you calculate an acid dissociation constant (Ka) of a weak acid?

11. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants
To find the Ka of a weak acid or the Kb of a weak base, substitute the measured concentrations of all the substances present at equilibrium into the expression for Ka or Kb.

12. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants
Acid Dissociation Constant
The dissociation constant, Ka, of ethanoic acid is calculated from the equilibrium concentrations of all of the molecules and ions in the solution.

13. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants
Dissociation of an acid (HA) in water yields H3O+ and A-. The bar graphs compare the extent of dissociation of strong, weak, and very weak acids. INTERPRETING GRAPHS a. Explain In the graph for the strong acid, why are the heights of the H3O+ and A- bars the same as the height of HA bar? b. Inferring In the graph for the weak acid, why is the height of the H3O+ bar the same as the distance from the top of the second HA bar to the dotted line? c. Apply Concepts Draw a bar graph for the dissociation of the weak diprotic acid, oxalic acid. Be sure to include the first and second dissociation.

14. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants

15. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants
Base Dissociation Constant
The dissociation constant, Kb, of ammonia is calculated from the equilibrium concentrations of all of the molecules and ions in the solution.

16. Calculating Dissociation Constants
19.3
Calculating Dissociation Constants
Concentration and Strength

17. 19.5

18. 19.5

19. 19.5

20. 19.5

21. Solve Problem 23 with the help of an interactive guided tutorial.
for Sample Problem 19.5
Problem Solving 19.23
Solve Problem 23 with the help of an interactive guided tutorial.

22. 19.3 Section Quiz.
19.3.

23. 19.3 Section Quiz.
1. H2S is considered to be a weak acid because it
is insoluble in water.
ionizes only slightly.
is completely ionized.
is dilute.

24. 19.3 Section Quiz.
2. Calcium hydroxide, Ca(OH)2, is a strong base because it
has a large Kb.
has a small Kb.
forms concentrated solutions.
is highly soluble in water.

25. 19.3 Section Quiz.
3. If the [H+] of a 0.205M solution of phenol (C6H5OH) at 25ºC is  10-6, what is the Ka for phenol? Phenol is monoprotic.
Ka = 2.67 x 10-11
Ka = 1.14 x 10-5
Ka = 5.48 x 10-12
Ka = 1.53 x 10-3

26. 19.3 Section Quiz.
4. The Ka of three acids is given below.
(1) 5.1  10–3
(2) 4.8  10–11
(3) 6.3  10–5
Put the acids in order from the strongest acid to the weakest acid.
1, 3, 2
2, 3, 1
3, 1, 2
2, 1, 3

27. 19.3 Section Quiz. 5. The Kb of four bases is given below.
(1) 7.41 x 10-5
(2) 1.78 x 10-5
(3) 4.27 x 10-4
(4) x 10-4
Put the bases in order from the strongest base to the weakest base.
2, 3, 4, 1
2, 1, 3, 4
4, 3, 1, 2
1, 4, 3, 2

28. END OF SHOW